I need help on this. I’ve done what I can but I’m not sure it’s right:-( Can someone please help me! If it’s wrong please show me the right way to do it.
7.62 g of iron reacts with 8.67 g of sulfur.
Fe + S --> FeS
a. Which reactant is the limiting reactant?
I think it should be:
7.62 g Fe * 1mol Fe* 88 g FeS/ 1mol FeS/ 56 g =12.0 g FeS
8.67 g S * 1 mol S* 88 g FeS/ 1mol FeS/ 32 g= 24 FeS
And Fe would be the limiting reactant?
b. What is the theoretical yield of the product? (In grams)
I think the answer is 8.26 g FeS
c. What is the percentage yield if only 8g of FeS is produced?
I have no idea how to do this last one.
7.62 g of iron reacts with 8.67 g of sulfur.
Fe + S --> FeS
a. Which reactant is the limiting reactant?
I think it should be:
7.62 g Fe * 1mol Fe* 88 g FeS/ 1mol FeS/ 56 g =12.0 g FeS
8.67 g S * 1 mol S* 88 g FeS/ 1mol FeS/ 32 g= 24 FeS
And Fe would be the limiting reactant?
b. What is the theoretical yield of the product? (In grams)
I think the answer is 8.26 g FeS
c. What is the percentage yield if only 8g of FeS is produced?
I have no idea how to do this last one.
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7.62 g of iron reacts with 8.67 g of sulfur.
Fe + S --> FeS
According to the coefficients in the balanced equation, 1 mole of Fe reacts with 1 mole of S to produce 1 mole of FeS
Number of moles of Fe = 7.62 ÷ 55.8 = 0.1366
Number of moles of S = 8.67 ÷ 32.1 = 0.2701
Since the number of moles of Fe is less than the number of moles of S, the Fe is the limiting reactant.
According to the coefficients in the balanced equation, 1 mole of Fe reacts with 1 mole of S to produce 1 mole of FeS. So, 0.1366 mole of Fe should react with 0.1366 mole of S, to produce 0.1366 mole of FeS.
Theoretical mass of S that should react = 0.1366 * 32.1 ≈ 4.38 grams
Theoretical mass of FeS that should be produced = 0.1366 * (55.8 + 32.1) ≈ 12.0 grams
OR
Theoretical mass of FeS = Mass of Fe + Theoretical mass of S
Theoretical mass of FeS = 7.62 + 4.38 = 12 g
% Yield = 100 * Actual mass ÷ Theoretical mass
If 8 g of FeS is produced:
% Yield of FeS = 100 * 8.0 ÷ 12.0 = 66⅔ %
Fe + S --> FeS
According to the coefficients in the balanced equation, 1 mole of Fe reacts with 1 mole of S to produce 1 mole of FeS
Number of moles of Fe = 7.62 ÷ 55.8 = 0.1366
Number of moles of S = 8.67 ÷ 32.1 = 0.2701
Since the number of moles of Fe is less than the number of moles of S, the Fe is the limiting reactant.
According to the coefficients in the balanced equation, 1 mole of Fe reacts with 1 mole of S to produce 1 mole of FeS. So, 0.1366 mole of Fe should react with 0.1366 mole of S, to produce 0.1366 mole of FeS.
Theoretical mass of S that should react = 0.1366 * 32.1 ≈ 4.38 grams
Theoretical mass of FeS that should be produced = 0.1366 * (55.8 + 32.1) ≈ 12.0 grams
OR
Theoretical mass of FeS = Mass of Fe + Theoretical mass of S
Theoretical mass of FeS = 7.62 + 4.38 = 12 g
% Yield = 100 * Actual mass ÷ Theoretical mass
If 8 g of FeS is produced:
% Yield of FeS = 100 * 8.0 ÷ 12.0 = 66⅔ %
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moles reactants-
Fe: 7.62 g/55.85 g/mole= 0.136 moles
S: 8.67 g/32 g/mole= 0.271 mole
from the bal. rxn., 1 mole Fe reacts with 1 mole of S, therefore, Fe is limitng reactant
theo. yield: 0.136 x 87.91 g mole FeS=11.96 g Fes
% yield= actual/theo. x 100
% yield= 8 g/12 g x 100
% yield= 66.7
Fe: 7.62 g/55.85 g/mole= 0.136 moles
S: 8.67 g/32 g/mole= 0.271 mole
from the bal. rxn., 1 mole Fe reacts with 1 mole of S, therefore, Fe is limitng reactant
theo. yield: 0.136 x 87.91 g mole FeS=11.96 g Fes
% yield= actual/theo. x 100
% yield= 8 g/12 g x 100
% yield= 66.7